Producing nitrogen and hydrogen mixtures



' are described.

l ll i iilil intent RALPH L. DODGE, OF CHARLESTON, WEST VIRGINIA, ASSIGNOR, BY M'ESNE ASSIGN- MENTS, TO 15. I. DU FONT DE NEMOURS A CORPORATION OF DELAWARE & COMPANY, OF WILMINGTON, DELAWARE,

rnonuome mrnoenn AND HYDROGEN MIXTURESi' No Drawing. Original application filed. April 29, 193Q,1 Seria1 No. Mil/AWL. Divided and thi's'application filed January 21, 1931. Serial No. 510,286. g i I i This invention relates to the production of gaseous mixtures of nitrogen and hydrogen and more particularly to the production of such mixtures by the catalytic decomposition of ammonia, as set forth in my co-pending application, Ser. No. 448,424, filed April. 29,

1930, of which the present application is, a

division. 1

It is known that ammonia can be decomposed into its elements, nitrogen and vhydro synthetic ammonia as the raw material, this.

is a convenient way of readily obtaining hydrogen of a high degree of purity which may advantageously be employed under circumst ances such that the presence of the relatively inert nitrogen is of little disadvantage.

Iron alone exhibits some activity as a catalyst for the thermal decomposition of am monia but when employed for any prolonged period at such elevated temperatures, say 500 to 700 C. for example, as are desirable for the effective conduct of the reaction, this material becomes powdered and sintered in such a way as to obstruct the passage of gas through the reaction tube. If, therefore, the decomposition of ammonia is to be effected continuously over a long period of time, it is necessary at rather frequent intervals to replace the iron with fresh material.

It is the object of the present invention to provide an improved process for producing gaseous mixtures of nitrogen and hydrogen by the thermal decomposition of ammonia, the process being characterized by the employment of improved catalysts possessing a high degree of activity and capable of use for long periods of time Without disintegration.

Other objects and advantages tion will be apparent as it is better understood by reference to the following specification in which its details and preferred embodiments of the invencombining a'catalyst containing iron together with one or more oxides of the elements comprising the groups aluminum, zirconium, chromium, magnesium and calcium; By employing catalysts of this composition it is possible to efl'ect the decomposition of ammonia more rapidly and at a lower temperature than with iron alone.

Although various methods may be used in the preparation of the catalyst and other ingredients than those named above may also be included if desired, I have found that for the best results the catalyst should be substantially free from elements of the alkali metal group or compounds thereof. For, although the alkali. metals and their compounds are frequently used with advantage in catalytic compositions and in fact, due to the methods and the raw materials commonly employed in catalyst manufacture one or more of these elements are likely to be present, my experience has shown that it is advisable to take precautions to avoid the presence of alkali metals in the catalyst. In other words, it is preferred to avoid using such methods of preparation as would involve, for instance, the addition of any of the catalyst ingredients in the form of an alkali metal salt or if such catalyst be employed, totake steps to eliminate the alkali metal from the catalyst before-it is used in the decomposition of ammonia. The presence of alkali metal in the catalyst tends to decrease the life thereof, apparently by sintering and fusing in such a way as to obstruct the free flow of gas through the body of contact materials: s v

The catalysts herein described and methods for the preparation of which are set forth in the following examples aremore active and generally satisfactory in the thermal de composition of ammonia 'than iron alone. For example, I have carried on the decomposi tion of ammonia for. as long as 500 hours without appreciable deterioratkm of the catalyst. ,While various methods of preparing the Ice catalysts may be employed and the conditions under which they are used in decomposing ammonia may be varied wit-hm wide limits,

7 the following examples are given to illustrate Ill -a nickel or nichrome tube surroundedby an electrical heater. \Vhen ammonia gas 1 is i (ill the manner of practicing the invention;

Example 1.Mix a solution of ferric sulphate with an equal volume of 10% solution of ammonium chromate and then add ammonium hydroxide to complete precipitation. Filter the precipitate, wash free from sulphates and dry. Form the dried material decomposition. of-ammonia it is disposed in passed over this catalyst at a temperature -within the range of 600 to700 C. the ammonia is decomposed into its elements and by suitably adjusting the rate of flow an efficient conversion of ammonia to nitrogen and hy- :lrogen may be obtained. Any undecoinposed ammonia may be removed fromthe gaseous products by one of the known ways, as, for

example, by absorption in water or an acid.

Ezra-721.1776 2.-A catalystadapted for use in the manner indicated under Example 1 may be prepared by adding approximately 3% by weight of magnesium oxide and 3% by weight of aluminum oxide to pure ierroso ferric oxide, the percentages being based on the total catalytic material calculated as oxide; Melt the oxide mixture, allow it to cool and crush and screen it to suitable size. The; catalyst is subjected to reduction before use.

Example 3.-The catalyst described in Example 1 may be replaced'by'one prepared by fusing terroso ferric oxide with 2% by weight of zirconium oxide. The molten mixture is allowed to cool, crushed, screened to suitable size and then reduced.

No explanation or theory is oflered as to any changes in physical form orcheniical composition. that may occur in the catalyst in the course of its reduction or during actual use. The term catalyst as employed in the claims is intended, theretore,-to include the contact mass as prepared as well as any modified form in which it may exist during the reaction. It should also be understood that, since it is generally recognized that the activity of substances as catalysts is a function of the chemical elements contained therein rather than of the particular type of compound employed, the term oxide as employed herein is to he considered as including oxides as such or as they may be present in chemical combination with other elements.

\Vhile the ienuierature range of GOO-700 C. indicated in the t'oregoing examples represents the preferred temperature range, the invention. is not limited to the utilization of these temperatures. The reaction can actually be initiated and carried on at lower temperatures, but for'efiicient operation of the process I prefer to employ the elevated temperatures named. I Higher temperatures may also beeniployed but,! generally speaking,

of the catalyst; U y I p l I, I

Various changes nay be made in the methoddescriloed without departing from the iny with some deterioration in the physical form vention'or sacrificing any of the'advantages. thereof. N v

" I claimr p 1.- Theprocess of producing a mixture of .nitrogen and hydrogenwhich comprises contacting gaseous ammonia. at an elevated temperature with a catalyst comprising iron and aluminum oxide.'-

" QJThe process of producing a mixture of nitrogen and hydrogen which comprises con tacting "gaseous ammonia at atemperature within the ra-nge of 600 to 709 C. with a catalyst comprising iron and aluminum oxide.

3. The process of producing a mixture of nitrogen and hydrogen :which comprises contacting gaseous ammonia at an elevated temperature with'a'cata-lyst consisting of iron and aluminum oxide, said catalyst being substantiall y free from alkali metal.

In testimony whereof, I atfix my signature.

RALPH DOD GE. 

